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CHEM103 Chapter Notes - Chapter 2.2: Conservation Of Mass, Antoine Lavoisier

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3 Jan 2016

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CHEM103 Full Course Notes

CHEM103 Full Course Notes

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2. 2 the observations that led to an atomic view of matter. The law of mass conservation: the total mass of substances does not change during a chemical reaction. The number of substances may change and, by definition, their properties must, but the total amount of matter remains constant. (lavoisier first stated this law on the basis of his combustion experiments) Mass conservation means that based on all chemical experience, matter cannot be created or destroyed. B/c the energy changes of chemical reactions are so small, for all practical purposes, mass is conserved. The law of definite (or constant) composition: no matter what its source, a particular compound is composed of the same elements in the same parts (fractions) by mass. The fraction by mass (mass fraction) is the part of the compound s mass that each element contributes. It is obtained by dividing the mass of each element by the mass of the compound.

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Chemical Reactions and Equations Learning objectives To observe physical and chemical properties associated with chemical changes To be able to give evidence for the occurrence of a chemical reaction To write a balanced chemical equation To identify areaction as a combination, decomposition, precipitation, single or double replacement, or combustion reaction ntroduction When a substance undergoes a physical change, it changes its appearance but not its composition. For example, when ice melts to form water, it undergoes a physical change from solid to liquid. In a chemical change, the composition of a substance is changed to give a new substance with different physical and chemical properties. For example, when silver tarnishes, the shiny silver (Ag) changes to a dull gray silver sulfide (AgaS). Not only has the chemical formula changed from Ag to Agus, but also the physical properties (shininess) of the substance have changed. Some examples of physical and chemical changes are listed in Table 1 below. Table 1. Comparison of Physical and Chemical Changes Examples of Physical changes Examples and Evidence of Chemical Changes Change in state (melting, freezing, evaporating Formation of a gas (bubbles) subliming) Formation of a solid (precipitate) Change in size Tearing Change in Color Heat is given off or absorbed A solid dissolving in a solvent In a chemical reaction, atoms in the reactants are rearranged to produce new combinations of atoms in the products. However, the total number of atoms of each element in the reactants is equal to the total number of atoms in the products. This is true according to the Law of Conservation of Mass, which states that the total mass remains constant during a chemical reaction. In other words, matter cannot be created or destroyed in a chemical reaction. In a chemical equation, the reactants are shown on the left and the products are on the right. An arrow in between indicates that a chemical reaction occurs. Finally, the physical state of each compound is designated in parentheses after the chemical formula. Solid, liquid, gas, and aqueous (dissolved in water) are shown as(s,(n,(g), and (aq), respectively.